What mass of #"KCl"# is contained in #"0.125 mols"# of #"KCl"#?

1 Answer
Truong-Son N.
Aug 18, 2015

You can figure this out by looking at the periodic table and finding potassium and chlorine. Or, by googling each element you can find out their atomic masses. Or, you could google the compound itself and find its overall molar mass.

Potassium is #K#, which is #38.098 "g/mol"#.
Chloride is the anion of Chlorine (or #Cl#), which is #35.453 "g/mol"#.

Thus, add to get the molar mass for #KCl#, which is #73.551 "g/mol"#.

So, just do a simple conversion. Since the units are #"g/mol"#, it means that you have #73.551 "g"# for every #"mol"# of #KCl#. So, if you only have #1/8# of a #"mol"#, then:

#0.125 cancel("mol" KCl) * (73.551 "g KCl")/cancel("mol KCl") ~~ color(blue)(9.1939 "g" "KCl")#

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